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Chemistry: The Central Science, 12e (Brown et al.)
Chapter 4 Aqueous Reactions and Solution Stoichiometry
4.1 Multiple Choice Questions
1) Of the species below, only __________ is not an electrolyte.
A) HCl
B) Rb2SO4
C) Ar
D) KOH
E) NaCl
2) The balanced molecular equation for complete neutralization of H2SO4 by KOH in aqueous solution
is __________.
A) 2H+ (aq) + 2OH- (aq) → 2 H2O (l)
B) 2H+ (aq) + 2KOH (aq) → 2 H2O (l) + 2K+ (aq)
C) H2SO4 (aq) + 2OH- (aq) → 2 H2O (l) + SO42- (aq)
D) H2SO4 (aq) + 2KOH (aq) → 2 H2O (l) + K2SO4 (s)
E) H2SO4 (aq) + 2KOH (aq) → 2 H2O (l) + K2SO4 (aq)
3) Aqueous potassium chloride will react with which one of the following in an exchange (metathesis)
reaction?
A) calcium nitrate
B) sodium bromide
C) lead nitrate
D) barium nitrate
E) sodium chloride
4) Aqueous solutions of a compound did not form precipitates with Cl-, Br-, I-, SO42- , CO32-, PO43-,
OH-, or S2-. This highly water-soluble compound produced the foul-smelling gas H2S when the
solution was acidified. This compound is __________.
A) Pb(NO3)2
B) (NH4)2S
C) KBr
D) Li2CO3
E) AgNO3
5) The net ionic equation for formation of an aqueous solution of NiI2 accompanied by evolution of
CO2 gas via mixing solid NiCO3 and aqueous hydriodic acid is __________.
A) 2NiCO3 (s) + HI (aq) → 2 H2O (l) + CO2 (g) + 2Ni2+ (aq)
B) NiCO3 (s) + I- (aq) → 2 H2O (l) + CO2 (g) + Ni2+ (aq) + HI (aq)
C) NiCO3 (s) + 2H+ (aq) → H2O (l) + CO2 (g) + Ni2+ (aq)
D) NiCO3 (s) + 2HI (aq) → 2 H2O (l) + CO2 (g) + NiI2 (aq)
E) NiCO3 (s) + 2HI (aq) → H2O (l) + CO2 (g) + Ni2+ (aq) + 2 I- (aq)
6) The net ionic equation for formation of an aqueous solution of Al(NO3)3 via mixing solid Al(OH)3
and aqueous nitric acid is __________.
A) Al(OH)3 (s) + 3HNO3 (aq) → 3 H2O (l) + Al(NO3)3 (aq)
B) Al(OH)3 (s) + 3NO3- (aq) → 3OH- (aq) + Al(NO3)3 (aq)
C) Al(OH)3 (s) + 3NO3- (aq) → 3OH- (aq) + Al(NO3)3 (s)
D) Al(OH)3 (s) + 3H+ (aq) → 3 H2O (l) + Al3+ (aq)
E) Al(OH)3 (s) + 3HNO3 (aq) → 3 H2O (l) + Al3+ (aq) + NO3- (aq)
7) Which of the following is soluble in water at 25 °C?
A) Fe3 (PO4)2
B) Fe(OH)2
C) Fe(NO3)2
D) FeCO3
E) FeS
3
8) Which of the following is insoluble in water at 25 °C?
A) Mg3(PO4)2
B) Na2S
C) (NH4)2CO3
D) Ca(OH)2
E) Ba(C2H3O2)2
9) When aqueous solutions of __________ are mixed, a precipitate forms.
A) NiBr2 and AgNO3
B) NaI and KBr
C) K2SO4 and CrCl3
D) KOH and Ba(NO3)2
E) Li2CO3 and CsI
10) Which one of the following compounds is insoluble in water?
A) Na2CO3
B) K2SO4
C) Fe(NO3)3
D) ZnS
E) AgNO3
11) Which one of the following compounds is insoluble in water?
A) K2SO4
B) Ca(C2H3O2)2
C) MgC2O4
D) ZnCl2
E) Mn(NO3)2
12) Which combination will produce a precipitate?
A) NaC2H3O2 (aq) and HCl (aq)
B) NaOH (aq) and HCl (aq)
C) AgNO3 (aq) and Ca(C2H3O2)2 (aq)
D) KOH (aq) and Mg(NO3)2 (aq)
E) NaOH (aq) and HCl (aq)
13) Which combination will produce a precipitate?
A) NH4OH (aq) and HCl (aq)
B) AgNO3 (aq) and Ca(C2H3O2)2 (aq)
C) NaOH (aq) and HCl (aq)
D) NaCl (aq) and H C2H3O2 (aq)
E) NaOH (aq) and Fe(NO3)2 (aq)
14) Which combination will produce a precipitate?
A) Pb(NO3)2 (aq) and HCl (aq)
B) Cu(NO3)2 (aq) and KC2H3O2 (aq)
C) KOH (aq) and HNO3 (aq)
D) AgC2H3O2 (aq) and HC2H3O2 (aq)
E) NaOH (aq) and Sr(NO3)2 (aq)
15) With which of the following will the ammonium ion form an insoluble salt?
A) chloride
B) sulfate
C) carbonate
D) sulfate and carbonate
E) none of the above
16) With which of the following will the potassium ion form an insoluble salt?
A) chloride
B) sulfate
C) carbonate
D) sulfate and carbonate
E) none of the above
17) The net ionic equation for the reaction between aqueous sulfuric acid and aqueous sodium hydroxide
is __________.
A) H+ (aq) + HSO4- (aq) + 2OH- (aq) → 2 H2O (l) + SO42- (aq)
B) H+ (aq) + HSO4- (aq) + 2 Na+ (aq) + 2OH- (aq) → 2 H2O (l) + 2Na+ (aq) + SO42- (aq)
C) SO42- (aq) + 2Na+ (aq) → 2Na+ (aq) + SO42- (aq)
D) H+ (aq) + OH- (aq) → H2O( l)
E) 2H+ (aq) + SO42- (aq) + 2Na+ (aq) + 2OH- (aq) → 2 H2O (l) + 2Na+ (aq) + SO42- (aq)
18) The net ionic equation for the reaction between aqueous nitric acid and aqueous sodium hydroxide is
__________.
A) H+ (aq) + HNO3 (aq) + 2OH- (aq) → 2 H2O (l) + NO3- (aq)
B) HNO3 (aq) + NaOH (aq) → NaNO3 (aq) + H2O (l)
C) H+ (aq) + OH- (aq) → H2O (l)
D) HNO3 (aq) + OH- (aq) → NO3- (aq) + H2O (l)
E) H+ (aq) + Na+ (aq) +OH- (aq) → H2O (l) + Na+ (aq)
19) The reaction between strontium hydroxide and chloric acid produces __________.
A) a molecular compound and a weak electrolyte
B) two weak electrolytes
C) two strong electrolytes
D) a molecular compound and a strong electrolyte
E) two molecular compounds
20) Which one of the following is a diprotic acid?
A) nitric acid
B) chloric acid
C) phosphoric acid
D) hydrofluoric acid
E) sulfuric acid
6
21) Which one of the following is a triprotic acid?
A) nitric acid
B) chloric acid
C) phosphoric acid
D) hydrofluoric acid
E) sulfuric acid
22) Which one of the following solutions will have the greatest concentration of hydroxide ions?
A) 0.300 M rubidium hydroxide
B) 0.100 M magnesium hydroxide
C) 0.100 M ammonia
D) 0.100 M beryllium hydroxide
E) 0.100 M hydrochloric acid
23) Which one of the following is a weak acid?
A) HNO3
B) HCl
C) HI
D) HF
E) HClO4
24) Which of the following are weak acids?
A) HF, HBr
B) HI, HNO3, HBr
C) HI, HF
D) HF
E) none of the above
25) A compound was found to be soluble in water. It was also found that addition of acid to an aqueous
solution of this compound resulted in the formation of carbon dioxide. Which one of the following
cations would form a precipitate when added to an aqueous solution of this compound?
A) NH4+
B) K+
C) Cr3+
D) Rb+
E) Na+
26) Which hydroxides are weak bases?
A) KOH, Ba(OH)2
B) Sr(OH)2, KOH, NaOH, Ba(OH)2
C) KOH, NaOH
D) KOH, NaOH, Ba(OH)2
E) None of these is a weak base.
27) The balanced reaction between aqueous potassium hydroxide and aqueous acetic acid is
__________.
A) KOH (aq) + HC2H3O2 (aq) → OH- (l) + H C2H3O2+ (aq) + K (s)
B) KOH (aq) + HC2H3O2 (aq) → H2O (l) + KC2H3O2 ( aq)
C) KOH (aq) + HC2H3O2 (aq) → H2C2H3O3 (aq) + K (s)
D) KOH (aq) + HC2H3O2 (aq) → KC2H3O3 (aq) + H2 (g)
E) KOH (aq) + HC2H3O2 (aq) → H2KC2H3O (aq) + O2 (g)
28) The balanced reaction between aqueous nitric acid and aqueous strontium hydroxide is __________.
A) HNO3 (aq) + Sr(OH)2 (aq) → Sr(NO3)2 (aq) + H2 (g)
B) HNO3 (aq) + Sr(OH)2 (aq) → H2O (l) + Sr(NO3)2 (aq)
C) HNO3 (aq) + SrOH (aq) → H2O (l) + SrNO3 (aq)
D) 2HNO3 (aq) + Sr(OH)2 (aq) → 2 H2O (l) + Sr(NO3)2 (aq)
E) 2HNO3 (aq) + Sr(OH)2 (aq) → Sr(NO3)2 (aq) + 2 H2 (g)
29) In which reaction does the oxidation number of oxygen increase?
A) Ba(NO3)2 (aq) + K2SO4 (aq) → BaSO4 (s) + 2 KNO3 (aq)
B) HCl (aq) + NaOH (aq) → NaCl (aq) + H2O (l)
C) MgO (s) + H2O (l) → Mg(OH)2 (s)
D) 2 SO2 (g) + O2 (g) → 2 SO3 (g)
E) 2 H2O (l) → 2 H2 (g) + O2 (g)
30) In which reaction does the oxidation number of hydrogen change?
A) HCl (aq) + NaOH (aq) → NaCl (aq) + H2O (l)
B) 2 Na (s) + 2 H2O (l) → 2 NaOH (aq) + H2 (g)
C) CaO (s) + H2O (l) → Ca(OH)2 (s)
D) 2 HClO4 (aq) + CaCO3 (s) → Ca(ClO4)2 (aq) + H2O (l) + CO2 (g)
E) SO2 (g) + H2O (l) → H2SO3 (aq)
31) In which species does sulfur have the highest oxidation number?
A) S8 (elemental form of sulfur)
B) H2S
C) SO2
D) H2SO3
E) K2SO4
32) In which species does nitrogen have the highest oxidation number?
A) N2
B) NH3
C) HNO2
D) NO2-
E) NaNO3
33) Which compound has the atom with the highest oxidation number?
A) CaS
B) Na3N
C) MgSO3
D) Al(NO2)3
E) NH4Cl
9
34) Of the choices below, which would be the best for the lining of a tank intended for use in storage of
hydrochloric acid?
A) copper
B) zinc
C) nickel
D) iron
E) tin
35) Which of these metals will be oxidized by the ions of cobalt?
A) nickel
B) tin
C) iron
D) copper
E) silver
36) Which of these metals will be oxidized by the ions of aluminum?
A) magnesium
B) zinc
C) chromium
D) iron
E) nickel
37) One method for removal of metal ions from a solution is to convert the metal to its elemental form
so it can be filtered out as a solid. Which metal can be used to remove aluminum ions from solution?
A) zinc
B) cobalt
C) lead
D) copper
E) none of these
38) Of the reactions below, only __________ is not spontaneous.
A) Mg (s) + 2HCl (aq) → MgCl2 (aq) + H2 (g)
B) 2Ag (s) + 2HNO3 (aq) → 2AgNO3 (aq) + H2 (g)
C) 2Ni (s) + H2SO4 (aq) → Ni2SO4 (aq) + H2 (g)
D) 2Al (s) + 6HBr (aq) → 2AlBr3 (aq) + 3 H2 (g)
E) Zn (s) + 2HI (aq) → ZnI2 (aq) + H2 (g)
39) Based on the activity series, which one of the reactions below will occur?
A) Zn (s) + MnI2 (aq) → ZnI2 (aq) + Mn (s)
B) SnCl2 (aq) + Cu (s) → Sn (s) + CuCl2 (aq)
C) 2AgNO3 (aq) + Pb (s) → 2Ag (s) + Pb(NO3)2 (aq)
D) 3Hg (l) + 2Cr(NO3)3 (aq) → 3Hg(NO3)2 + 2Cr (s)
E) 3FeBr2 (aq) + 2Au (s) → 3Fe (s) + 2AuBr3 (aq)
40) Based on the activity series, which one of the reactions below will occur?
A) Fe (s) + ZnCl2 (aq) → FeCl2 (aq) + Zn (s)
B) Mn (s) + NiCl2 (aq) → MnCl2 (aq) + Ni (s)
C) Pb (s) + NiI2 (aq) → PbI2 (aq) + Ni (s)
D) SnBr2 (aq) + Cu (s) → CuBr2 (aq) + Sn (s)
E) None of the reactions will occur.
41) The net ionic equation for the dissolution of zinc metal in aqueous hydrobromic acid is __________.
A) Zn (s) + 2Br- (aq) → ZnBr2 (aq)
B) Zn (s) + 2HBr (aq) → ZnBr2 (aq) + 2H+ (aq)
C) Zn (s) + 2HBr (aq) → ZnBr2 (s) + 2H+ (aq)
D) Zn (s) + 2H+ (aq) → Zn2+ (aq) + H2 (g)
E) 2Zn (s) + H+ (aq) → 2Zn2+ (aq) + H2 (g)
42) Sodium does not occur in nature as Na (s) because __________.
A) it is easily reduced to Na-
B) it is easily oxidized to Na+
C) it reacts with water with great difficulty
D) it is easily replaced by silver in its ores
E) it undergoes a disproportionation reaction to Na- and Na+
11
43) Zinc is more active than cobalt and iron but less active than aluminum. Cobalt is more active than
nickel but less active than iron. Which of the following correctly lists the elements in order of
increasing activity?
A) Co < Ni < Fe < Zn < Al
B) Ni < Fe < Co < Zn < Al
C) Ni < Co < Fe < Zn < Al
D) Fe < Ni < Co < Al < Zn
E) Zn < Al < Co < Ni < Fe
44) Oxidation is the __________ and reduction is the __________.
A) gain of oxygen, loss of electrons
B) loss of oxygen, gain of electrons
C) loss of electrons, gain of electrons
D) gain of oxygen, loss of mass
E) gain of electrons, loss of electrons
45) Oxidation and __________ mean essentially the same thing.
A) activity
B) reduction
C) metathesis
D) decomposition
E) corrosion
46) Oxidation cannot occur without __________.
A) acid
B) oxygen
C) water
D) air
E) reduction
47) Which of the following is an oxidation-reduction reaction?
A) Cu (s) + 2AgNO3 (aq) → 2Ag (s) + Cu(NO3)2 (aq)
B) HCl (aq) + NaOH (aq) → H2O (l) + NaCl (aq)
C) AgNO3 (aq) + HCl (aq) → AgCl (s) + HNO3 (aq)
D) Ba(C2H3O2)2 (aq) + Na2SO4 (aq) → BaSO4 (s) + 2NaC2H3O2 (aq)
E) H2CO3 (aq) + Ca(NO3)2 (aq) → 2HNO3 (aq) + CaCO3 (s)
48) Which of the following reactions will not occur as written?
A) Zn (s) + Pb(NO3)2 (aq) → Pb (s) + Zn(NO3)2 (aq)
B) Mg (s) + Ca(OH)2 (aq) → Ca (s) + Mg(OH)2 (aq)
C) Sn (s) + 2AgNO3 (aq) → 2Ag (s) + Sn(NO3)2 (aq)
D) Co (s) + 2AgCl (aq) → 2Ag (s) + CoCl2 (aq)
E) Co (s) + 2HI (aq) → H2 (g) + CoI2 (aq)
49) Which one of the following is a correct expression for molarity?
A) mol solute/L solvent
B) mol solute/mL solvent
C) mmol solute/mL solution
D) mol solute/kg solvent
E) μmol solute/L solution
50) Which one of the following is not true concerning 2.00 L of 0.100 M solution of Ca3(PO4)2?
A) This solution contains 0.200 mol of Ca3(PO4)2.
B) This solution contains 0.800 mol of oxygen atoms.
C) 1.00 L of this solution is required to furnish 0.300 mol of Ca2+ ions.
D) There are 6.02 × 1022 phosphorus atoms in 500.0 mL of this solution.
E) This solution contains 6.67 × 10-2 mol of Ca2+.
51) A 0.200 M K2SO4 solution is produced by __________.
A) dilution of 250.0 mL of 1.00 M K2SO4 to 1.00 L
B) dissolving 43.6 g of K2SO4 in water and diluting to a total volume of 250.0 mL
C) diluting 20.0 mL of 5.00 M K2SO4 solution to 500.0 mL
D) dissolving 20.2 g of K2SO4 in water and diluting to 250.0 mL, then diluting 25.0 mL of this solution
to a total volume of 500.0 mL
E) dilution of 1.00 mL of 250 M K2SO3 to 1.00 L
13
52) Which solution has the same number of moles of NaOH as 50.00 mL of 0.100M solution of NaOH?
A) 20.00 mL of 0.200M solution of NaOH
B) 25.00 mL of 0.175M solution of NaOH
C) 30.00 mL of 0.145M solution of NaOH
D) 50.00 mL of 0.125M solution of NaOH
E) 100.00 mL of 0.0500M solution of NaOH
53) Which solution has the same number of moles of KCl as 75.00 mL of 0.250M solution of KCl?
A) 20.0 mL of 0.200M solution of KCl
B) 25.0 mL of 0.175M solution of KCl
C) 129 mL of 0.145M solution of KCl
D) 50.0 mL of 0.125M solution of KCl
E) 100 mL of 0.0500M solution of KCl
54) What are the respective concentrations (M) of Fe3+ and I- afforded by dissolving 0.200 mol FeI3 in
water and diluting to 725 mL?
A) 0.276 and 0.828
B) 0.828 and 0.276
C) 0.276 and 0.276
D) 0.145 and 0.435
E) 0.145 and 0.0483
55) What are the respective concentrations (M) of Mg+2 and C2H3O2- afforded by dissolving 0.600
mol Mg(C2H3O2)2 in water and diluting to 135 mL?
A) 0.444 and 0.889
B) 0.0444 and 0.0889
C) 0..889 and 0.444
D) 0.444 and 0.444
E) 4.44 and 8.89
56) What are the respective concentrations (M) of Cu+2 and Cl- afforded by dissolving 0.200 mol
CuCl2 in water and diluting to 345 mL?
A) 0.200 and 0.200
B) 0.580 and 1.16
C) 0.200 and 0.400
D) 1.16 and 2.32
E) 0.580 and 0.290
57) A tenfold dilution of a sample solution can be obtained by taking __________.
A) 1 part sample and 9 parts solvent
B) 1 part sample and 10 parts solvent
C) 9 parts sample and 1 part solvent
D) 10 parts sample and 1 part solvent
E) 99 parts sample and 1 part solvent
58) Mixing 10.00 mL of an aqueous solution with 10.00 mL of water represents a __________.
A) crystallization
B) neutralization
C) twofold dilution
D) tenfold dilution
E) titration
59) You are given two clear solutions of the same unknown monoprotic acid, but with different
concentrations. Which statement is true?
A) There is no chemical method designed to tell the two solutions apart.
B) It would take more base solution (per milliliter of the unknown solution) to neutralize the more
concentrated solution.
C) A smaller volume of the less concentrated solution contains the same number of moles of the acid
compared to the more concentrated solution.
D) If the same volume of each sample was taken, then more base solution would be required to
neutralize the one with lower concentration.
E) The product of concentration and volume of the less concentrated solution equals the product of
concentration and volume of the more concentrated solution.
60) A 0.100 M solution of __________ will contain the highest concentration of potassium ions.
A) potassium phosphate
B) potassium hydrogen carbonate
C) potassium hypochlorite
D) potassium iodide
E) potassium oxide
61) Which solution contains the largest number of moles of chloride ions?
A) 10.0 mL of 0.500M BaCl2
B) 4.00 mL of 1.000M NaCl
C) 7.50 mL of 0.500M FeCl3
D) 25.00 mL of 0.400M KCl
E) 30.00 mL of 0.100M CaCl2
62) What volume (mL) of a concentrated solution of sodium hydroxide (6.00 M) must be diluted to 200.
mL to make a 1.50 M solution of sodium hydroxide?
A) 0.0500
B) 50.0
C) 45.0
D) 800.
E) 0.800
63) What volume (mL) of a concentrated solution of magnesium chloride (9.00 M) must be diluted to
350. mL to make a 2.75 M solution of magnesium chloride?
A) 2.75
B) 50.0
C) 45.0
D) 107
E) 350
64) What volume (mL) of a concentrated solution of sodium hydroxide (6.00 M) must be diluted to
200.0 mL to make a 0.880 M solution of sodium hydroxide?
A) 2.64
B) 176
C) 26.4
D) 29.3
E) 50.0
65) What mass (g) of potassium chloride is contained in 430.0 mL of a potassium chloride solution that
has a chloride ion concentration of 0.193 M?
A) 0.0643
B) 0.0830
C) 12.37
D) 0.386
E) 6.19
66) What volume (ml) of a 3.45 M lead nitrate solution must be diluted to 450.0 ml to make a 0.990 M
solution of lead nitrate?
A) 129
B) 109
C) 101
D) 56
E) 45
67) What mass (g) of barium iodide is contained in 250 mL of a barium iodide solution that has an
iodide ion concentration of 0.193 M?
A) 9.44
B) 18.9
C) 0.024
D) 0.048
E) 37.7
68) What mass (g) of AgBr is formed when 35.5 mL of 0.184 M AgNO3 is treated with an excess of
aqueous hydrobromic acid?
A) 1.44
B) 1.23
C) 53.6
D) 34.5
E) 188
17
69) What mass (g) of CaF2 is formed when 47.8 mL of 0.334 M NaF is treated with an excess of
aqueous calcium nitrate?
A) 1.25
B) 0.472
C) 2.49
D) 0.943
E) 0.623
70) What volume (mL) of 0.135 M NaOH is required to neutralize 13.7 mL of 0.129 M HCl?
A) 13.1
B) 0.24
C) 14.3
D) 0.076
E) 6.55
71) What volume (L) of 0.250 M HNO3 is required to neutralize a solution prepared by dissolving
17.5 g of NaOH in 350 mL of water?
A) 50.0
B) 0.44
C) 1.75
D) 0.070
E) 1.75 ×
72) An aliquot (28.7 mL) of a KOH solution required 31.3 mL of 0.118 M HCl for neutralization.
What mass (g) of KOH was in the original sample?
A) 1.64
B) 7.28
C) 0.173
D) 0.207
E) 0.414
73) The point in a titration at which the indicator changes is called the __________.
A) setpoint
B) indicator point
C) standard point
D) endpoint
E) volumetric point
74) Which of the following would require the largest volume of 0.100 M sodium hydroxide solution for
neutralization?
A) 10.0 mL of 0.0500 M phosphoric acid
B) 20.0 mL of 0.0500 M nitric acid
C) 5.0 mL of 0.0100 M sulfuric acid
D) 15.0 mL of 0.0500 M hydrobromic acid
E) 10.0 mL of 0.0500 M perchloric acid
75) Which one of the following substances is produced during the reaction of an acid with a metal
hydroxide?
A) H2
B) H2O
C) CO2
D) NaOH
E) O2
76) A 36.3 mL aliquot of 0.0529 M H2SO4 (aq) is to be titrated with 0.0411 M NaOH (aq). What
volume (mL) of base will it take to reach the equivalence point?
A) 93.4
B) 46.7
C) 187
D) 1.92
E) 3.84
77) A 13.8 mL aliquot of 0.176 M H3PO4 (aq) is to be titrated with 0.110 M NaOH (aq). What volume
(mL) of base will it take to reach the equivalence point?
A) 7.29
B) 22.1
C) 199
D) 66.2
E) 20.9
19
78) What volume (mL) of 7.48 × 10-2 M perchloric acid can be neutralized with 115 mL of 0.244 M
sodium hydroxide?
A) 125
B) 8.60
C) 188
D) 750
E) 375
79) What volume (mL) of 7.48 × 10-2 M phosphoric acid can be neutralized with 115 mL of 0.244 M
sodium hydroxide?
A) 125
B) 375
C) 750
D) 188
E) 75.0
80) __________ is an oxidation reaction.
A) Ice melting in a soft drink
B) Table salt dissolving in water for cooking vegetables
C) Rusting of iron
D) The reaction of sodium chloride with lead nitrate to form lead chloride and sodium nitrate
E) Neutralization of HCl by NaOH
4.2 Bimodal Questions
1) A strong electrolyte is one that __________ completely in solution.
A) reacts
B) associates
C) disappears
D) ionizes
2) A weak electrolyte exists predominantly as __________ in solution.
A) atoms
B) ions
C) molecules
D) electrons
E) an isotope
3) Which of the following are strong electrolytes?
20
HCl
HC2H3O2NH3
KCl
A) HCl, KCl
B) HCl, NH3, KCl
C) HCl, HC2H3O2, NH3, KCl
D) HCl, HC2H3O2, KCl
E) HC2H3O2, KCl
4) Which of the following are weak electrolytes?
HCl
HC2H3O2
NH3
KCl
A) HCl, KCl
B) HCl, HC2H3O2, NH3, KCl
C) HC2H3O2, KCl
D) HC2H3O2, NH3
E) HCl, HC2H3O2, KCl
5) What are the spectator ions in the reaction between KOH (aq) and HNO3 (aq)?
A) K+ and H+
B) H+ and OH-
C) K+ and NO3-
D) H+ and NO3-
E) OH- only
6) What are the spectator ions in the reaction between KCl (aq) and AgNO3 (aq)?
A) K+ and Ag+
B) Ag+ and Cl-
C) K+ and NO3-
D) Ag+ and NO3-
E) K+ only
7) What are the spectator ions in the reaction between Mg(OH)2 (aq) and HCl (aq)?
A) Mg+2 and H+
